05. Gibbs Energy Change and Equilibrium
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Thermodynamics

273069 For $\mathrm{CaCO}_3$ (s) $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})$ at $927^{\circ} \mathrm{C}$
$\Delta \mathbf{H}=176 \mathrm{~kJ} \mathrm{~mol}^{-1}$ then $\Delta \mathrm{E}$ is :

1 $180 \mathrm{~kJ}$
2 $186.4 \mathrm{~kJ}$
3 $166.0 \mathrm{~kJ}$
4 $160 \mathrm{~kJ}$
BCECE-2006
Thermodynamics

273080 For the chemical reaction, $X \to Y$, the standard reaction Gibbs energy depends on temperature $\mathbf{T}$ (in $\mathrm{K}$ ) as
$\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\left(\right.$ in $\left.\mathrm{kJ} \mathrm{mol}^{-1}\right)=120-\frac{3}{8} T$
The major component of the reaction mixture at $T$ is

1 $\mathrm{Y}$ if $\mathrm{T}=280 \mathrm{~K}$
2 $\mathrm{X}$ if $\mathrm{T}=350 \mathrm{~K}$
3 $\mathrm{X}$ if $\mathrm{T}=315 \mathrm{~K}$
4 $\mathrm{Y}$ if $\mathrm{T}=300 \mathrm{~K}$
JEE Main-2019, Shift-I
Thermodynamics

273071 For a chemical reaction, $\Delta G$ is always less than $\operatorname{zero}(\Delta \mathbf{G}<0)$ if

1 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are positive
2 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are negative
3 $\Delta \mathrm{H}$ is negative and $\mathrm{T} \Delta \mathrm{S}$ is positive
4 $\Delta \mathrm{H}$ is positive and $\mathrm{T} \Delta \mathrm{S}$ is negative
CG PET -2019
Thermodynamics

273074 For a spontaneous reaction, the $\Delta \mathbf{G}$, equilibrium constant (K) and $E_{\text {cell }}^{\circ}$ will be respectively

1 - ve, $>1,-$ ve
2 - ve $,<1,-$ ve
3 $+\mathrm{ve},>1,-\mathrm{ve}$
4 $-\mathrm{ve},>1,+\mathrm{ve}$
AIEEE-2005
NEET DIGITAL LIBRARY
Thermodynamics

273069 For $\mathrm{CaCO}_3$ (s) $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})$ at $927^{\circ} \mathrm{C}$
$\Delta \mathbf{H}=176 \mathrm{~kJ} \mathrm{~mol}^{-1}$ then $\Delta \mathrm{E}$ is :

1 $180 \mathrm{~kJ}$
2 $186.4 \mathrm{~kJ}$
3 $166.0 \mathrm{~kJ}$
4 $160 \mathrm{~kJ}$
BCECE-2006
Thermodynamics

273080 For the chemical reaction, $X \to Y$, the standard reaction Gibbs energy depends on temperature $\mathbf{T}$ (in $\mathrm{K}$ ) as
$\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\left(\right.$ in $\left.\mathrm{kJ} \mathrm{mol}^{-1}\right)=120-\frac{3}{8} T$
The major component of the reaction mixture at $T$ is

1 $\mathrm{Y}$ if $\mathrm{T}=280 \mathrm{~K}$
2 $\mathrm{X}$ if $\mathrm{T}=350 \mathrm{~K}$
3 $\mathrm{X}$ if $\mathrm{T}=315 \mathrm{~K}$
4 $\mathrm{Y}$ if $\mathrm{T}=300 \mathrm{~K}$
JEE Main-2019, Shift-I
Thermodynamics

273071 For a chemical reaction, $\Delta G$ is always less than $\operatorname{zero}(\Delta \mathbf{G}<0)$ if

1 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are positive
2 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are negative
3 $\Delta \mathrm{H}$ is negative and $\mathrm{T} \Delta \mathrm{S}$ is positive
4 $\Delta \mathrm{H}$ is positive and $\mathrm{T} \Delta \mathrm{S}$ is negative
CG PET -2019
Thermodynamics

273074 For a spontaneous reaction, the $\Delta \mathbf{G}$, equilibrium constant (K) and $E_{\text {cell }}^{\circ}$ will be respectively

1 - ve, $>1,-$ ve
2 - ve $,<1,-$ ve
3 $+\mathrm{ve},>1,-\mathrm{ve}$
4 $-\mathrm{ve},>1,+\mathrm{ve}$
AIEEE-2005
Join With Us for More Updates
Thermodynamics

273069 For $\mathrm{CaCO}_3$ (s) $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})$ at $927^{\circ} \mathrm{C}$
$\Delta \mathbf{H}=176 \mathrm{~kJ} \mathrm{~mol}^{-1}$ then $\Delta \mathrm{E}$ is :

1 $180 \mathrm{~kJ}$
2 $186.4 \mathrm{~kJ}$
3 $166.0 \mathrm{~kJ}$
4 $160 \mathrm{~kJ}$
BCECE-2006
Thermodynamics

273080 For the chemical reaction, $X \to Y$, the standard reaction Gibbs energy depends on temperature $\mathbf{T}$ (in $\mathrm{K}$ ) as
$\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\left(\right.$ in $\left.\mathrm{kJ} \mathrm{mol}^{-1}\right)=120-\frac{3}{8} T$
The major component of the reaction mixture at $T$ is

1 $\mathrm{Y}$ if $\mathrm{T}=280 \mathrm{~K}$
2 $\mathrm{X}$ if $\mathrm{T}=350 \mathrm{~K}$
3 $\mathrm{X}$ if $\mathrm{T}=315 \mathrm{~K}$
4 $\mathrm{Y}$ if $\mathrm{T}=300 \mathrm{~K}$
JEE Main-2019, Shift-I
Thermodynamics

273071 For a chemical reaction, $\Delta G$ is always less than $\operatorname{zero}(\Delta \mathbf{G}<0)$ if

1 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are positive
2 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are negative
3 $\Delta \mathrm{H}$ is negative and $\mathrm{T} \Delta \mathrm{S}$ is positive
4 $\Delta \mathrm{H}$ is positive and $\mathrm{T} \Delta \mathrm{S}$ is negative
CG PET -2019
Thermodynamics

273074 For a spontaneous reaction, the $\Delta \mathbf{G}$, equilibrium constant (K) and $E_{\text {cell }}^{\circ}$ will be respectively

1 - ve, $>1,-$ ve
2 - ve $,<1,-$ ve
3 $+\mathrm{ve},>1,-\mathrm{ve}$
4 $-\mathrm{ve},>1,+\mathrm{ve}$
AIEEE-2005
For More Updates join with Us
Thermodynamics

273069 For $\mathrm{CaCO}_3$ (s) $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})$ at $927^{\circ} \mathrm{C}$
$\Delta \mathbf{H}=176 \mathrm{~kJ} \mathrm{~mol}^{-1}$ then $\Delta \mathrm{E}$ is :

1 $180 \mathrm{~kJ}$
2 $186.4 \mathrm{~kJ}$
3 $166.0 \mathrm{~kJ}$
4 $160 \mathrm{~kJ}$
BCECE-2006
Thermodynamics

273080 For the chemical reaction, $X \to Y$, the standard reaction Gibbs energy depends on temperature $\mathbf{T}$ (in $\mathrm{K}$ ) as
$\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\left(\right.$ in $\left.\mathrm{kJ} \mathrm{mol}^{-1}\right)=120-\frac{3}{8} T$
The major component of the reaction mixture at $T$ is

1 $\mathrm{Y}$ if $\mathrm{T}=280 \mathrm{~K}$
2 $\mathrm{X}$ if $\mathrm{T}=350 \mathrm{~K}$
3 $\mathrm{X}$ if $\mathrm{T}=315 \mathrm{~K}$
4 $\mathrm{Y}$ if $\mathrm{T}=300 \mathrm{~K}$
JEE Main-2019, Shift-I
Thermodynamics

273071 For a chemical reaction, $\Delta G$ is always less than $\operatorname{zero}(\Delta \mathbf{G}<0)$ if

1 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are positive
2 $\Delta \mathrm{H}$ and $\mathrm{T} \Delta \mathrm{S}$ both are negative
3 $\Delta \mathrm{H}$ is negative and $\mathrm{T} \Delta \mathrm{S}$ is positive
4 $\Delta \mathrm{H}$ is positive and $\mathrm{T} \Delta \mathrm{S}$ is negative
CG PET -2019
Thermodynamics

273074 For a spontaneous reaction, the $\Delta \mathbf{G}$, equilibrium constant (K) and $E_{\text {cell }}^{\circ}$ will be respectively

1 - ve, $>1,-$ ve
2 - ve $,<1,-$ ve
3 $+\mathrm{ve},>1,-\mathrm{ve}$
4 $-\mathrm{ve},>1,+\mathrm{ve}$
AIEEE-2005
NEET DIGITAL LIBRARY